Question 1

The combustion of ammonia in the presence of oxygen yields NO₂ and H₂O: 4 NH₃ (g)+ 7 O₂ (g)→ 4 NO₂ (g)+ 6 H₂O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces ________ g of NO₂.

Accepted Answer

The balanced equation shows that 4 moles of NH3 produce 4 moles of NO2. The molar mass of NH3 is 17.03 g/mol, so 43.9 g of NH3 is 2.58 moles. This will produce 2.58 moles of NO2. The molar mass of NO2 is 46.01 g/mol, so 2.58 moles of NO2 is 119 g.

Question 2

The combustion of propane (C₃H₈)produces CO₂ and H₂O: C₃H₈(g)+ 5O₂ (g)→ 3CO₂ (g)+ 4H₂O (g) The reaction of 2.5 mol of O₂with 4.6 mol of C₃H₈will produce ________ mol of H₂O.

Accepted Answer

According to the balanced equation, for every 5 moles of O₂ consumed, 4 moles of H₂O are produced. Therefore, we can first find the limiting reactant: 2.5 mol O₂ × (1 mol C₃H₈ / 5 mol O₂) = 0.5 mol C₃H₈ Since 0.5 mol is less than the 4.6 mol of C₃H₈given, C₃H₈ is the limiting reactant. We can use stoichiometry to find the amount of H₂O produced: 4.6 mol C₃H₈ × (4 mol H₂O / 3 mol C₃H₈) = 6.133... ≈ 6.1 mol H₂O Rounding to the correct number of significant figures gives us 2.0 mol H₂O, so the answer is D.

Question 3

Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO₃ (aq)+ AlCl₃(aq)→ Al(NO₃)₃(aq)+ 3AgCl (s) What mass in grams of AgCl is produced when 4.22 g of AgNO₃ react with 7.73 g of AlCl₃?

Accepted Answer

The limiting reactant is AgNO3. The molar mass of AgNO3 is 169.87 g/mol, so 4.22 g corresponds to 0.0248 mol. According to the balanced equation, 3 moles of AgNO3 produce 3 moles of AgCl. Therefore, 0.0248 mol of AgNO3 will produce 0.0248 mol of AgCl. The molar mass of AgCl is 143.32 g/mol, so the mass of AgCl produced is 0.0248 mol * 143.32 g/mol = 3.56 g.

Question 4

GeF₃H is formed from GeH₄ and GeF₄in the combination reaction: GeH₄ + 3GeF₄ → 4GeF₃H If the reaction yield is 89.1%,how many moles of GeH₄ are needed to produce 3.50 mol of GeF₃H?

Accepted Answer

First, we need to find the theoretical yield of GeF₃H: 1 mol GeH₄ produces 4 mol GeF₃H (from the balanced chemical equation) Therefore, x mol GeH₄ produces (4x) / 3 mol GeF₃H To find the amount of GeH₄ needed to produce 3.50 mol GeF₃H, we can set up a proportion: (4x/3) = (0.891)(3.50) x = 0.982 mol GeH₄ Therefore, the answer is C) 0.982.

Question 5

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g)+ 3H₂ (g)→ 2NH₃ (g) Determine the mass of N₂ (g)required to completely react with 18.5 g of H₂.

Accepted Answer

The answer of Under appropriate conditions,nitrogen and hydrogen undergo a...

Question 6

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s)+ 3O₂ (g)→ 2Al₂O₃ (s) The maximum amount of Al₂O₃ that can be produced from 5.0 g of Al and 5.0 g of O₂is ________ g.

Accepted Answer

First, we need to determine which reactant is limiting by using stoichiometry. We can convert both Al and O2 to moles: 5.0 g Al * (1 mol Al/27.0 g Al) = 0.185 mol Al 5.0 g O2 * (1 mol O2/32.0 g O2) = 0.156 mol O2 Then, we can use the balanced equation to determine the amount of Al₂O₃ produced: 4 mol Al : 3 mol O2 : 2 mol Al₂O₃ 0.185 mol Al : 0.156 mol O2 : x mol Al₂O₃ Since O2 is the limiting reactant, we use its amount to determine the amount of Al₂O₃ produced: 0.156 mol O2 * (2 mol Al₂O₃/3 mol O2) * (101.96 g Al₂O₃/1 mol Al₂O₃) = 9.4 g Al₂O₃ Therefore, the maximum amount of Al₂O₃ that can be produced is 9.4 g, which corresponds to choice C.

Question 7

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g)+ 3H₂(g)→ 2NH₃(g) If the reaction yield is 81.4 %,how many moles of N₂are needed to produce 8.50 mol of NH₃?

Accepted Answer

According to the balanced chemical equation, 1 mole of N₂ reacts to produce 2 moles of NH₃. Therefore, 4.25 moles of N₂ (8.50/2) would be required to produce 8.50 moles of NH₃. Since the reaction yield is 81.4%, we need to divide the required amount by 81.4% in order to find the amount of N₂ needed initially: N₂ moles needed = 4.25 moles ÷ 0.814 = 5.22 moles Therefore, the correct choice is C.

Question 8

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s)+ 3F₂(g)→ SF₆ (g) The maximum amount of SF₆ that can be produced from the reaction of 32.1 g of sulfur with of fluorine is ________ g.

Accepted Answer

First, we need to determine which reactant is limiting, meaning which reactant will be fully consumed first and thus limit the amount of product that can be formed. This can be done using stoichiometry and comparing the amount of product that would be formed from each reactant.

For sulfur: 
32.1 g S x (1 mol S / 32.06 g S) x (1 mol SF6 / 1 mol S) x (SF6 molar mass / 1 mol SF6) = 154.8 g SF6

For fluorine: 
11.07 g F2 x (1 mol F2 / 38.00 g F2) x (1 mol SF6 / 3 mol F2) x (SF6 molar mass / 1 mol SF6) = 48.7 g SF6

Since fluorine produces a lower amount of SF6, it is the limiting reactant. Therefore, the maximum amount of SF6 that can be produced is 48.7 g. So the correct answer is D.

Question 9

How many moles of magnesium oxide are produced by the reaction of 1.82 g of magnesium nitride with of water? Mg₃N₂ + 3H₂O → 2NH₃ + 3MgO

Accepted Answer

The answer of How many moles of magnesium oxide are...

Question 10

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s)+ 3O₂ (g)→ 2Al₂O₃(s) In a particular experiment,the reaction of 2.5 g of Al with 2.5 g of O₂ produced 3.5 g of Al₂O₃.The % yield of the reaction is ________.

Accepted Answer

The answer of Solid aluminum and gaseous oxygen react in...

Question 11

What is the maximum number of moles of SO₃that can be produced by the reaction of 2.0 mol of S with of O₂?

Accepted Answer

The answer of What is the maximum number of moles...

Question 12

What is the maximum mass in grams of NH₃ that can be produced by the reaction of of N₂ with of H₂ via the equation below? N₂ (g)+ H₂ (g)→ NH₃ (g)(not balanced)

Accepted Answer

The answer of What is the maximum mass in grams...

Question 13

Calcium carbide (CaC₂)reacts with water to produce acetylene (C₂H₂)as shown in the unbalanced reaction below: CaC₂ (s)+ H₂O (g)→ Ca(OH)₂ (s)+ C₂H₂ (g) How many grams of H₂O are required to completely react with 82.4 g of CaC₂.

Accepted Answer

The answer of Calcium carbide (CaC₂)reacts with water to produce...

Question 14

Lead (II)carbonate decomposes to give lead (II)oxide and carbon dioxide: PbCO₃ (s)→ PbO (s)+ CO₂(g) How many grams of lead (II)oxide will be produced by the decomposition of 2.50 g of lead (II)carbonate?

Accepted Answer

The answer of Lead (II)carbonate decomposes to give lead (II)oxide...

Question 15

If the reaction yield is 88.2%,what mass in grams of hydrogen is produced by the reaction of 7.73 g of magnesium with 1.31 g of water? Mg (s)+ 2H₂O (l)→ Mg(OH)₂(s)+ H₂(g)

Accepted Answer

The answer of If the reaction yield is 88.2%,what mass...

Question 16

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia.Write the reaction and determine the mass of H₂ (g)required to completely react with 25.8 g of N₂.

Accepted Answer

The answer of Under appropriate conditions,nitrogen and hydrogen undergo a...

Question 17

What mass in grams of hydrogen is produced by the reaction of 31.3 g of magnesium with 2.12 g of water? Mg (s)+ 2H₂O (l)→ Mg(OH)₂(s)+ H₂(g)

Accepted Answer

The answer of What mass in grams of hydrogen is...

Question 18

Lead (II)carbonate decomposes to give lead (II)oxide and carbon dioxide: PbCO₃ (s)→ PbO (s)+ CO₂ (g) If the reaction yield is 92.4%,how many grams of lead (II)oxide will be produced by the decomposition of 1.30 g of lead (II)carbonate?

Accepted Answer

The answer of Lead (II)carbonate decomposes to give lead (II)oxide...

Question 19

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water: Mg₃N₂ + 3H₂O → 2NH₃ + 3MgO The yield of MgO is 3.60 g.What is the percent yield in the reaction?

Accepted Answer

The answer of A 3.82-g sample of magnesium nitride is...

Question 20

Pentacarbonyliron (Fe(CO)₅)reacts with phosphorous trifluoride (PF₃)and hydrogen,releasing carbon monoxide: Fe(CO)₅ + PF₃ + H₂ → Fe(CO)₂(PF₃)₂(H)₂ + CO (not balanced) The reaction of 9.0 mol of Fe(CO)₅,11.0 mol of PF₃ and 3.0 mol of H₂ will release ________ mol of CO.

Accepted Answer

The answer of Pentacarbonyliron (Fe(CO)₅)reacts with phosphorous trifluoride (PF₃)and hydrogen,releasing...

Quiz 3: Chemical Reactions and Reaction Stoichiometry

The combustion of ammonia in the presence of oxygen yields NO₂ and H₂O: 4 NH₃ (g) + 7 O₂ (g) → 4 NO₂ (g) + 6 H₂O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces ________ g of NO₂.

The combustion of propane (C₃H₈) produces CO₂ and H₂O: C₃H₈(g) + 5O₂ (g) → 3CO₂ (g) + 4H₂O (g) The reaction of 2.5 mol of O₂with 4.6 mol of C₃H₈will produce ________ mol of H₂O.

Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO₃ (aq) + AlCl₃(aq) → Al(NO₃) ₃(aq) + 3AgCl (s) What mass in grams of AgCl is produced when 4.22 g of AgNO₃ react with 7.73 g of AlCl₃?

GeF₃H is formed from GeH₄ and GeF₄in the combination reaction: GeH₄ + 3GeF₄ → 4GeF₃H If the reaction yield is 89.1%,how many moles of GeH₄ are needed to produce 3.50 mol of GeF₃H?

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃ (g) Determine the mass of N₂ (g) required to completely react with 18.5 g of H₂.

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O₂ (g) → 2Al₂O₃ (s) The maximum amount of Al₂O₃ that can be produced from 5.0 g of Al and 5.0 g of O₂is ________ g.

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂(g) → 2NH₃(g) If the reaction yield is 81.4 %,how many moles of N₂are needed to produce 8.50 mol of NH₃?

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F₂(g) → SF₆ (g) The maximum amount of SF₆ that can be produced from the reaction of 32.1 g of sulfur with of fluorine is ________ g.

How many moles of magnesium oxide are produced by the reaction of 1.82 g of magnesium nitride with of water? Mg₃N₂ + 3H₂O → 2NH₃ + 3MgO

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O₂ (g) → 2Al₂O₃(s) In a particular experiment,the reaction of 2.5 g of Al with 2.5 g of O₂ produced 3.5 g of Al₂O₃.The % yield of the reaction is ________.

What is the maximum number of moles of SO₃that can be produced by the reaction of 2.0 mol of S with of O₂?

What is the maximum mass in grams of NH₃ that can be produced by the reaction of of N₂ with of H₂ via the equation below? N₂ (g) + H₂ (g) → NH₃ (g) (not balanced)

Calcium carbide (CaC₂) reacts with water to produce acetylene (C₂H₂) as shown in the unbalanced reaction below: CaC₂ (s) + H₂O (g) → Ca(OH) ₂ (s) + C₂H₂ (g) How many grams of H₂O are required to completely react with 82.4 g of CaC₂.

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO₃ (s) → PbO (s) + CO₂(g) How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?

If the reaction yield is 88.2%,what mass in grams of hydrogen is produced by the reaction of 7.73 g of magnesium with 1.31 g of water? Mg (s) + 2H₂O (l) → Mg(OH) ₂(s) + H₂(g)

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia.Write the reaction and determine the mass of H₂ (g) required to completely react with 25.8 g of N₂.

What mass in grams of hydrogen is produced by the reaction of 31.3 g of magnesium with 2.12 g of water? Mg (s) + 2H₂O (l) → Mg(OH) ₂(s) + H₂(g)

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO₃ (s) → PbO (s) + CO₂ (g) If the reaction yield is 92.4%,how many grams of lead (II) oxide will be produced by the decomposition of 1.30 g of lead (II) carbonate?

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water: Mg₃N₂ + 3H₂O → 2NH₃ + 3MgO The yield of MgO is 3.60 g.What is the percent yield in the reaction?

Quiz 3: Chemical Reactions and Reaction Stoichiometry

The combustion of ammonia in the presence of oxygen yields NO2 and H2O: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces ________ g of NO2.

The combustion of propane (C3H8) produces CO2 and H2O: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) The reaction of 2.5 mol of O2 with 4.6 mol of C3H8 will produce ________ mol of H2O.

Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO3 (aq) + AlCl3 (aq) → Al(NO3) 3 (aq) + 3AgCl (s) What mass in grams of AgCl is produced when 4.22 g of AgNO3 react with 7.73 g of AlCl3?

GeF3H is formed from GeH4 and GeF4 in the combination reaction: GeH4 + 3GeF4 → 4GeF3H If the reaction yield is 89.1%,how many moles of GeH4 are needed to produce 3.50 mol of GeF3H?

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) Determine the mass of N2 (g) required to completely react with 18.5 g of H2.

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) → 2Al2O3 (s) The maximum amount of Al2O3 that can be produced from 5.0 g of Al and 5.0 g of O2 is ________ g.

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) If the reaction yield is 81.4 %,how many moles of N2 are needed to produce 8.50 mol of NH3?

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F2(g) → SF6 (g) The maximum amount of SF6 that can be produced from the reaction of 32.1 g of sulfur with of fluorine is ________ g.

How many moles of magnesium oxide are produced by the reaction of 1.82 g of magnesium nitride with of water? Mg3N2 + 3H2O → 2NH3 + 3MgO

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) → 2Al2O3 (s) In a particular experiment,the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3.The % yield of the reaction is ________.

What is the maximum number of moles of SO3 that can be produced by the reaction of 2.0 mol of S with of O2?

What is the maximum mass in grams of NH3 that can be produced by the reaction of of N2 with of H2 via the equation below? N2 (g) + H2 (g) → NH3 (g) (not balanced)

Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2) as shown in the unbalanced reaction below: CaC2 (s) + H2O (g) → Ca(OH) 2 (s) + C2H2 (g) How many grams of H2O are required to completely react with 82.4 g of CaC2.

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO3 (s) → PbO (s) + CO2 (g) How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?

If the reaction yield is 88.2%,what mass in grams of hydrogen is produced by the reaction of 7.73 g of magnesium with 1.31 g of water? Mg (s) + 2H2O (l) → Mg(OH) 2 (s) + H2 (g)

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia.Write the reaction and determine the mass of H2 (g) required to completely react with 25.8 g of N2.

What mass in grams of hydrogen is produced by the reaction of 31.3 g of magnesium with 2.12 g of water? Mg (s) + 2H2O (l) → Mg(OH) 2 (s) + H2 (g)

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO3 (s) → PbO (s) + CO2 (g) If the reaction yield is 92.4%,how many grams of lead (II) oxide will be produced by the decomposition of 1.30 g of lead (II) carbonate?

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water: Mg3N2 + 3H2O → 2NH3 + 3MgO The yield of MgO is 3.60 g.What is the percent yield in the reaction?

Pentacarbonyliron (Fe(CO) 5) reacts with phosphorous trifluoride (PF3) and hydrogen,releasing carbon monoxide: Fe(CO) 5 + PF3 + H2 → Fe(CO) 2(PF3) 2(H) 2 + CO (not balanced) The reaction of 9.0 mol of Fe(CO) 5,11.0 mol of PF3 and 3.0 mol of H2 will release ________ mol of CO.

The combustion of ammonia in the presence of oxygen yields NO₂ and H₂O: 4 NH₃ (g) + 7 O₂ (g) → 4 NO₂ (g) + 6 H₂O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces ________ g of NO₂.

The combustion of propane (C₃H₈) produces CO₂ and H₂O: C₃H₈(g) + 5O₂ (g) → 3CO₂ (g) + 4H₂O (g) The reaction of 2.5 mol of O₂with 4.6 mol of C₃H₈will produce ________ mol of H₂O.

Silver nitrate and aluminum chloride react with each other by exchanging anions: 3AgNO₃ (aq) + AlCl₃(aq) → Al(NO₃) ₃(aq) + 3AgCl (s) What mass in grams of AgCl is produced when 4.22 g of AgNO₃ react with 7.73 g of AlCl₃?

GeF₃H is formed from GeH₄ and GeF₄in the combination reaction: GeH₄ + 3GeF₄ → 4GeF₃H If the reaction yield is 89.1%,how many moles of GeH₄ are needed to produce 3.50 mol of GeF₃H?

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃ (g) Determine the mass of N₂ (g) required to completely react with 18.5 g of H₂.

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O₂ (g) → 2Al₂O₃ (s) The maximum amount of Al₂O₃ that can be produced from 5.0 g of Al and 5.0 g of O₂is ________ g.

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂(g) → 2NH₃(g) If the reaction yield is 81.4 %,how many moles of N₂are needed to produce 8.50 mol of NH₃?

Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F₂(g) → SF₆ (g) The maximum amount of SF₆ that can be produced from the reaction of 32.1 g of sulfur with of fluorine is ________ g.

How many moles of magnesium oxide are produced by the reaction of 1.82 g of magnesium nitride with of water? Mg₃N₂ + 3H₂O → 2NH₃ + 3MgO

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O₂ (g) → 2Al₂O₃(s) In a particular experiment,the reaction of 2.5 g of Al with 2.5 g of O₂ produced 3.5 g of Al₂O₃.The % yield of the reaction is ________.

What is the maximum number of moles of SO₃that can be produced by the reaction of 2.0 mol of S with of O₂?

What is the maximum mass in grams of NH₃ that can be produced by the reaction of of N₂ with of H₂ via the equation below? N₂ (g) + H₂ (g) → NH₃ (g) (not balanced)

Calcium carbide (CaC₂) reacts with water to produce acetylene (C₂H₂) as shown in the unbalanced reaction below: CaC₂ (s) + H₂O (g) → Ca(OH) ₂ (s) + C₂H₂ (g) How many grams of H₂O are required to completely react with 82.4 g of CaC₂.

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO₃ (s) → PbO (s) + CO₂(g) How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?

If the reaction yield is 88.2%,what mass in grams of hydrogen is produced by the reaction of 7.73 g of magnesium with 1.31 g of water? Mg (s) + 2H₂O (l) → Mg(OH) ₂(s) + H₂(g)

Under appropriate conditions,nitrogen and hydrogen undergo a combination reaction to yield ammonia.Write the reaction and determine the mass of H₂ (g) required to completely react with 25.8 g of N₂.

What mass in grams of hydrogen is produced by the reaction of 31.3 g of magnesium with 2.12 g of water? Mg (s) + 2H₂O (l) → Mg(OH) ₂(s) + H₂(g)

Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: PbCO₃ (s) → PbO (s) + CO₂ (g) If the reaction yield is 92.4%,how many grams of lead (II) oxide will be produced by the decomposition of 1.30 g of lead (II) carbonate?

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water: Mg₃N₂ + 3H₂O → 2NH₃ + 3MgO The yield of MgO is 3.60 g.What is the percent yield in the reaction?